Multiple Choice
Identify the
choice that best completes the statement or answers the question.
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1.
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According to this chemical reaction, which is the number of grams of Fe produced
from 14 moles of H2?
Fe3O4 (cr) + 4 H2 (g)
® 3 Fe (cr) + 4 H2O (l)
a. | 587 g | c. | 4862 g | b. | 2431 g | d. | 22.1 g |
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2.
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Which is the correct mole ratio of K3PO4 to KNO3
in the chemical reaction
Mg(NO3)2 + K3PO4 ®Mg3(PO4)2 + KNO3?
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3.
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Which is the correct mole ratio for aluminum chloride to chlorine in the
chemical reaction
AlCl3 + Br2 ®
AlBr3 + Cl2?
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4.
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How many moles of KBr will be produced from 7 moles of
BaBr2?
BaBr2 + K2SO4 ®
KBr + BaSO4
a. | 1 mole | c. | 14 moles | b. | 7 moles | d. | 3.5 moles |
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5.
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Which is the number of moles of carbon dioxide produced from the complete
combustion of 5.42 moles of ethanol?
C2H6O + O2 ® CO2 + H2O
a. | 5.42 moles | c. | 10.84 moles | b. | 2.71 moles | d. | 16.3 moles |
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6.
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How many grams of water are produced when 2.50 mol oxygen reacts with
hydrogen?
H2 + O2 ® H2O
a. | 45.0 g | c. | 90.0 g | b. | 22.5 g | d. | 3.6 g |
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7.
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How many grams of O2 are required to produce 358.5 grams of ZnO?
2Zn + O2 ® 2ZnO
a. | 1302 g | c. | 29.1 g | b. | 14.5 g | d. | 70.5 g |
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8.
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How many grams of chlorine gas can be produced from the decomposition of 73.4 g.
of AuCl3 by this reaction:
2AuCl3 ® 2 Au + 3
Cl2
a. | 25.7 g | c. | 11.4 g | b. | 33.6 g | d. | 195.3 g |
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9.
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A chemical reaction can theoretically produce 137.5 grams of product, but in
actuality 112.9 grams are produced. Which is the percent yield for this reaction?
a. | 82.1% | c. | 24.6% | b. | 62.0 g | d. | 17.9% |
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10.
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A reaction was predicted to produce 32.4 grams of a compound. When the product
was measured, there were only 26.1 grams made. What is the percent yield of this reaction?
a. | 80.6% | c. | 24.1% | b. | 6.3% | d. | 58.5% |
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11.
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How many grams of H 2O will be produced if 750 grams of Fe are
produced?  a. | 17.9 g | c. | 563 g | b. | 322 g | d. | 241 g |
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12.
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How many grams of Fe 3O 4 are required to react completely
with 300 grams of H 2?  a. | 2096 g | c. | 8681 g | b. | 1.54 g | d. | 37.5 g |
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13.
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Which is NOT an assumption of matter made by the kinetic molecular theory of
gases?
a. | Gas particles are small and take up little volume relative to the volume of the space
around them. | b. | The kinetic energy of particles is determined by their mass and their
velocity. | c. | When particles collide, their total energy is decreased. | d. | Gas particles are
widely dispersed and therefore are not affected significantly by attractive or repulsive
forces. |
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14.
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A sample of three mixed gases is at 632.0 mmHg. If the partial pressure of
CO2 is 124.3 mmHg and the partial pressure of N2 is 461.9 mmHg, what is the
partial pressure of O2?
a. | 760 mmHg | c. | 173.8 mmHg | b. | 45.8 mmHg | d. | 128 mmHg |
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15.
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Of the forces listed, which is strongest?
a. | covalent | c. | dispersion | b. | dipole-dipole | d. | hydrogen |
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16.
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Which is true regarding intermolecular forces?
a. | A hydrogen bond is a specialized type of dispersion force. | b. | Hydrogen bonds can
form with any atom in Groups 15, 16, or 17. | c. | The only forces holding nonpolar compounds
together are dispersion forces. | d. | Substances with strong intermolecular forces
tend to have very low boiling points. |
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17.
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Which is the term used to describe the energy required to increase the surface
area of a liquid?
a. | deposition | c. | surface tension | b. | viscosity | d. | surfactant |
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18.
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Which change in state requires that energy be added to the substance?
a. | freezing | c. | condensing | b. | deposition | d. | vaporizing |
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19.
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Which is the state change that occurs when a solid becomes a gas without
becoming a liquid first?
a. | vaporization | c. | deposition | b. | sublimation | d. | freezing |
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20.
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Above 33 K, no amount of pressure will liquefy hydrogen gas. At this
temperature, 1290 kPa are required to liquefy hydrogen. Which is the term used to refer to this
combination of pressure and temperature?
a. | deposition point | c. | triple point | b. | critical point | d. | vapor pressure |
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21.
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Which of the following changes requires an input
of thermal energy? a. | Freezing | c. | Evaporation | b. | Deposition | d. | Condensation |
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22.
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A gas particle of mass 5.31 ´ 10 
kg has a velocity of 1.00  10 2 m/s. What is the kinetic
energy of the molecule? a. | 5.31 ´ 10 kg
m2/s2 | c. | 2.65 ´ 10
kg m2/s2 | b. | 5.31 ´ 10 kg m2/s2 | d. | 10.6 ´ 10 kg
m2/s2 |
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23.
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A mixture of oxygen, hydrogen, and water vapor has a total pressure of 684 mm
Hg. The partial pressure of oxygen is 380 mm Hg and that of hydrogen is 0.100 atm. What is the
partial pressure of water vapor?
a. | 304 mm Hg | c. | 684 mm Hg | b. | 228 mm Hg | d. | 690 mm Hg |
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24.
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Which of the following about an ice cube floating in a glass of water is
correct?
a. | The temperature of the ice cube increases. | b. | The temperature of
the ice cube decreases. | c. | The temperature of the ice cube remains
constant. | d. | The temperature of the ice cube will fluctuate. |
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25.
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Which type of crystalline solid has atoms surrounded by mobile valence
electrons?
a. | atomic | c. | metallic | b. | covalent network | d. | molecular |
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26.
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Which law describes the proportional relationship between the pressure and
volume of a gas?
a. | Boyle’s Law | c. | Gay-Lussac’s Law | b. | Charles’s
Law | d. | Natural
Law |
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27.
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At an ocean depth of 10.0 m, a diver’s lung capacity is 2.40 L. The air
temperature is 32.0°C and the pressure is 101.30 kPa. What is the volume of the diver’s
lungs at the same depth, at a temperature of 21.0°C and a pressure of 141.20 kPa?
a. | 1.12 L | c. | 1.78 L | b. | 1.66 l | d. | 4.86 L |
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28.
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An ethylene gas torch requires 3200 L of gas at 3.00 atm. What will be the
pressure of the gas if ethylene is supplied by a 250.0 L tank?
a. | 0.231 atm | c. | 38.4 atm | b. | 2.34 atm | d. | 45.4 atm |
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29.
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Four liters of gas at atmospheric pressure is compressed into a 0.85L cylinder.
What is the pressure of the compressed gas if its temperature remains constant?
a. | 0.15 atm | c. | 3.4 atm | b. | 0.21 atm | d. | 4.7 atm |
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30.
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The _____ in a balanced equation specify volume ratios for gaseous reactants and
products.
a. | constants | c. | masses | b. | coefficients | d. | variables |
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31.
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A sample of oxygen gas has a volume of 150.0 mL when its pressure is .947 atm.
What will the volume of the gas in Figure 13.8 be if the temperature remains constant?
a. | 72 mL | c. | 216 mL | b. | 144 mL | d. | 288 mL |
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32.
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A sample of neon gas occupies a volume of 752 mL at 25°C. What volume will
the gas occupy at 50°C if the pressure remains constant?
a. | 204 mL | c. | 815 mL | b. | 408 mL | d. | 8150 mL |
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33.
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A helium-filled balloon has a volume of 50.0 L at 25°C and 1.08 atm. What
volume will it have at .855 atm and 10.0°C?
a. | 15.0 L | c. | 60.0 L | b. | 30.0 L | d. | 120.0 L |
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34.
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What quantity of gas, in moles, is contained in 2.21 L at STP?
a. | .0454 mol | c. | .1974 mol | b. | .0987 mol | d. | .2948 mol |
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35.
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What volume does .0685 mol of gas occupy at STP?
a. | .3707 mol | c. | 1.53 L | b. | .7515 mol | d. | 3.06 L |
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36.
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According to Gay-Lussac’s law:
a. | pressure is inversely proportional to volume at constant
temperature. | b. | pressure is directly proportional to temperature at constant
volume. | c. | volume is inversely proportional to temperature at constant
pressure. | d. | volume is directly proportional to temperature at constant
pressure. |
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37.
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Calculate the hydrogen ion concentration of an aqueous solution, given the
concentration of hydroxide ions is 1 ´ 10-5 M and the ion
constant for water is 1 ´ 10-14.
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38.
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When acids react with metals, they produce _____ gas.
a. | hydrogen | c. | sulfur | b. | nitrogen | d. | oxygen |
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39.
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A basic solution contains more _____ ions than hydrogen.
a. | oxygen | c. | hydroxide | b. | nitrogen | d. | sulfide |
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40.
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A _____ is produced when a base accepts a hydrogen ion from an acid.
a. | conjugate acid | c. | acid | b. | conjugate base | d. | base |
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41.
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What is the pH of blood, given the hydrogen ion concentration is 4.0 ´ 10-8 M?
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42.
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An acid that can donate only one hydrogen ion is called a _____ acid.
a. | monoprotic | c. | triprotic | b. | diprotic | d. | polyprotic |
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43.
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In the Bronsted-Lowry model of acids and bases, a(n) _____ is a hydrogen donor
and a(n) _____ is a hydrogen acceptor.
a. | acid, base | c. | conjugate acid, conjugate base | b. | base,
acid | d. | conjugate base,
conjugate acid |
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44.
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Which model states that an acid is a substance that contains hydrogen and
ionizes to produce hydrogen ions?
a. | Arrhenius | c. | Lewis | b. | Bronsted-Lowry | d. | Hydrogen |
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45.
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What is the ph of 0.45 M of H2SO4?
a. | 0.0045 | c. | 0.45 | b. | 0.045 | d. | 4.50 |
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46.
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What is the hydrogen ion concentration of 0.050 M
H3PO4?
a. | 0.015 M | c. | 1.50 M | b. | 0.15 M | d. | 15.0 M |
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47.
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A solution that contains equal concentrations of hydrogen and hydroxide ions is
_____.
a. | an acid | c. | neutral | b. | a base | d. | ionized |
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48.
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The pH scale allows scientists to define the acidity of a substance on a scale
of _____.
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49.
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Identify the acid and conjugate base pair in the following equation:   H 3O + + F  a. | HF & H20 | c. | HF &
F- | b. | HF & H30 | d. | H20 & H3O+ |
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50.
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An acid that has more than one ionizable hydrogen atom is called a _____
acid.
a. | monoprotic | c. | triprotic | b. | diprotic | d. | polyprotic |
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